0.2 moles of ${\text{H}}_{\text{2}}{\text{SO}}_{\text{4}}$ reacts with 0.2 moles of KOH in aqueous solution. Heat liberated during the process is 

Gram equivalent weight of strong acid =  $\text{0.2}\left(2\right)=4$
Gram equivalent weight of strong base =  $0.2\left(1\right)=0.2$
Heat liberated =  $0.2\left(-57.3\text{\hspace{0.17em}KJ}\right)$
                            = 11.46 KJ